1. Find the area under the curve between X =0 and 0.5 by numerical integration method such as the trapezoidal rule.

Mole Fraction ( X)	Potential (V)	Area (V)
0	0.250
0.01	0.230
0.02	0.203
0.04	0.162
0.08	0.125
0.1	0.110
0.2	0.073
0.4	0.030
0.48	0.016
0.5	0
	AVERAGE AREA (V)

2. Use Equation 7 to calculate the change entropy of mixing for a 50:50 mixture of the two 0.1 M solutions, and Equation 8 to find the molar entropy of mixing (Delta S mix,m). Compare your results with the theoretical values for a pseudo-ideal solution (Equation 3). When comparing Equation 3 with Equation 8, since you are finding the molar entropy (mixing one mole with one mole), nA = nB = 1 (or n = 2). When comparing Equation 3 with Equation 7, use nA = nB = 0.0025 mol (or n = 0.0050 mol).

3. In order to estimate the error in Delta S mix,m, you will need to find an estimate for the uncertainty in the area under the curve ( integration from 0 to 0.5 of EdX ). One way to do this is to estimate the error in the potential readings from the meter and to calculate the errors in the mole fraction (X) from the volumes measured for each mixture. If these uncertainties are added to the E and X coordinates of each point, a curve of a slightly greater area is generated, and the difference between the two areas can be taken as an estimate of the error in the area.

4. Considering the uncertainties in the graph area and the temperature, estimate the error in your value of Delta S mix,m, and thus report the correctly rounded value of Delta S mix,m +- the correctly rounded error, quoting the relevant temperature. Based on this error value, state whether your result agrees with the theoretical value for Delta S mix,m.

Smix=nR(XAlnXA+XBlnXB)=R(nAlnXA+nBlnXB) Gmix=c0VF00.5EdXSmix=TGmix=Tc0VF00.5EdX